30/12/2015 1 Energetics of metabolism Dr. Bódis Emőke October 7, 2015 JJ9 Why do we study difficult thermodynamics? The laws and principles of the thermodynamics describe the characteristics of matter- and energy flow of the different biochemical systems. - From these we can determine the direction of a spontaneous reaction. The 0. law of the thermodynamics (equilibrium and stability) If system A is in thermal equilibrium with system C, and system B is in thermal equilibrium with system C, then system A is in thermal equilibrium with system B. Two systems are said to be in thermal equilibrium if, when they are placed in ``thermal contact'' (basically, contact that permits the exchange of energy between them), their state variables do not change.
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30/12/2015
1
Energetics of metabolism
Dr. Bódis Emőke
October 7, 2015
JJ9
Why do we study difficult thermodynamics?
The laws and principles of the thermodynamics describe the characteristics of matter- and energy flow of the different biochemical systems.
- From these we can determine the direction of a spontaneous reaction.
The 0. law of the thermodynamics (equilibrium and stability)
If system A is in thermal equilibrium with system C, and system B is in thermal equilibrium with system C, then system A is in thermal equilibrium with system B.
Two systems are said to be in thermal equilibrium if, when they are placed in ``thermal contact'' (basically, contact that permits the exchange of energy between them), their state variables do not change.
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The I. law of the thermodynamic (conservation of energy)
ΔU = U2-U1 = Q + W
Energy can be converted from one form to another with the interaction of heat, work and internal energy. Energy can be changed from one form to another, but it cannot be created or destroyed.
BUT! In biological systems instead of internal energy it is more useful to apply ENTHALPY.
H = U + pVΔH = ΔU + pΔV = Q + W + pΔV = Q - pΔV + pΔV = Q
ΔH: Enthalpy change is the amount of heat content used or released in a system at constant pressure. (ΔU: Internal energy change is the amount of heat content used or released in a system at constant volume. )
HpVU
The II. Law of the thermodynamics (The direction of the processes)
Systems tend to proceed from ordered (low-entropy or low-probability) states to disordered (high-entropy or high-probability) states.
ΔQ = T ΔS
Heat transferred in a process change the entropy of the system.
Entropy represents energy dispersion:large number of molecular motions is relatable to quantized states (microstate)
S = k ln W = k ln (W2-W1)
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A termodinamika III. főtétele
Tökeletes kristalyos, tiszta anyagok entrópiaja (vegyuleteke is!) T = 0 K-en nulla.
Következmenye: T= 0 K-en ismerjuk az entrópia abszolut erteketDE! Biológiai folyamatokban az entrópia valtozas hasznosabb, mint az abszolut entrópia.
Pl: ΔG = ΔH – TΔS
A III. főtetel statisztikus magyarazata: S = k ln W egyenletből T = 0 K hőmersekleten a tökeletesen kristalyos anyagok reszecskeimind a leheto legalacsonyabb energiaju allapotban vannak
W = 1 es S = 0
A legalacsonyabb mert hőmerseklet a termeszetben 1 K (Boomerang csillagködben, 5000 fenyevnyire tőlunk, a Kentaur csillagkepben)
Egy reakció csak akkorspontan, ha a szabad energia
negatív!
It is usefull to apply for biological systems.
Question: Will the reaction proceed in the direction written?
1. The thermodynamic condition: Gibbs free energy must decrease.
Gibbs free energy: measures the "usefulness" or process-initiating work obtainable from a thermodynamic system at constant temperature and pressure.
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2. The reaction kinetic condition: the reactants must decrease the activation energy
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The catabolic ways are convergent, the anabolic ways are divergent.
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First period of the cellular respiration: Glycolysis
aroses 2 pyruvate molecules.
From 1 glucose molecule
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Pyruvate, a versatile metabolite
The final product of glycolysisCan be used in several ways
Oxygen is present (aerobic condition): pyruvate is oxidized and will be the acetyl group of acetyl-CoA and will further metabolized in the tricarboxylic acid cycle
A szabad energia valtozas bőven fedezi a 2 ATP szinteziset:
(61 / 183,6) * 100% = 33,2 %
(A felszabaduló energia 33,2 %-a fordítódik a 2 ATP szintezisere.)
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Why does Glycolysis occur? Are the thermodynamic and kinetic conditions necessary for the reactions met?
The first phase of Glycolysis
The first phase of Glycolysis: First energy priming reaction
Kinase: enzyme responsible for transferring the γ-phosphate of ATP to moleculesHexokinase: phosphorylate hexose sugars (C-6)
The first and third steps of the Glycolysis pathway will be primed with energy from hydrolysis of 2 ATP so that at the end of Glycolysis 4 ATP will be formed (net 2 ATP)
- 2 ATP binding sites- Low concentration of ATP: ATP binds to the high
affinity binding site (ATP at active site)- High concentration of ATP: : ATP binds also to the
low affinity binding site (ATP at regulatory site) glycolysis “turns off”
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Fourth step of Glycolysis
Fourth step of Glycolysis: concentration-dependent reaction
Fructose-Bisphosphate aldolase: claves between C3-C4 carbons yield two triose phosphates
Concentration-dependent reaction: - in vitro: the reaction does not proceed effectively from left to right
(ΔG positive: 23,97 kJ/mol)- in vivo: efficient
(ΔG negative: -0,23 kJ/mol
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Seventh step of Glycolysis
ADPMg2+
phosphate
Seventh step of Glycolysis: Synthesis of the first two ATPs
- Phosphoglycerate kinase: phophorylation of ADP (substrate-level phophorylation )- Two ATP were consumed in the first phase of Glycolysis , the Phosphoglycerate kinase reaction “pays off” the ATP debt created by the priming reactions- In living cells: ΔG : -0,1 kJ/mol
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Tenth (last) step of Glycolysis
Tenth (last) step of Glycolysis: Synthesis of the second two ATPs
Catalysator : Pyruvate kinasePresence of Mg2+ es K+ are necessary 1. step: phosphorylation of ADP2. step: enol-ketone conversion
Highly favorable and spontaneous conversion of the enol to the more stable keto form following the phosphorylation group transfer step.